as air filled in cycle tube and hen we done small hole it will lose its all air slowly slowly
One example of gas effusion is the release of a gas through a small hole in a container, such as when air slowly escapes from a balloon. Another example would be the diffusion of gas molecules through a porous membrane, like the way oxygen and carbon dioxide diffuse in and out of our lungs during respiration.
The movement of gas through a small hole into an area of lower pressure is diffusion.
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No
The rate of effusion is inversely related to the square root of the molar mass. Or stated another way, the larger or heavier the gas, the slower the effusion rate. Nitrogen gas (N2) has a molar mass of 28 g/mole and oxygen gas (O2) has a molar mass of 32 g/mole. Nitrogen will diffuse faster. rate N2/rate O2 = sqrt 32/sqrt 28 = 5.66/5.29 = 1.07. So, N2 effuses 1.07x faster than O2, or 7% faster. For more information on this, look up Graham's Law of Effusion.
The slowest rate of effusion will be exhibited by the gas with the highest molar mass. For example, Xenon will diffuse at a slower rate than Helium, and chlorine will diffuse at a slower rate than fluorine.
The movement of gas through a small hole into an area of lower pressure is diffusion.
Graham's law of effusion.
Graham's law of effusion states that the rate of effusion of a gas is inversely proportional to the square root of its molar mass. In other words, lighter gases effuse or diffuse at a faster rate than heavier gases under the same conditions.
A process related to diffusion is effusion, the process by which a gas escapes from a container into a vacuum through a small hole. The rate of effusion is also related to root mean square velocity-heavier molecules effuse more slowly than lighter ones. The rate of effusion-the amount of gas that effused in a given time- is inversely proportional to the square root of the molar mass of the gas.
Graham's law states that the rate of effusion of a gas is inversely proportional to the square root of its molecular weight.Graham's law states that the rate of effusion of a gas is inversely proportional to the square root of its molecular weight.
EFFUSION
No
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50000
effusion is the process where individual molecules flow through a hole without collisions between molecules. effusion is the process where the gas molecules are passed through a small opening to an evacuated chamber
The larger the particle size, the slower it will diffuse. This is given by Graham's Law of effusion which states that the rate of effusion is inversely related to the square root of the molar mass of the gas.
The rate of effusion is inversely related to the square root of the molar mass. Or stated another way, the larger or heavier the gas, the slower the effusion rate. Nitrogen gas (N2) has a molar mass of 28 g/mole and oxygen gas (O2) has a molar mass of 32 g/mole. Nitrogen will diffuse faster. rate N2/rate O2 = sqrt 32/sqrt 28 = 5.66/5.29 = 1.07. So, N2 effuses 1.07x faster than O2, or 7% faster. For more information on this, look up Graham's Law of Effusion.